State whether each of the following will increase,decrease or unchange when catalyst is added to the reaction and give an explanation for your answer please a) rate of reaction b)activation energy c)reaction enthalpy d)equilibrium of reaction

A catalyst lowers the activation energy, generally through the formation of an intermediate complex. A catalyst does not change delta H nor Keq.

a) When a catalyst is added to a reaction, it typically increases the rate of reaction. This occurs because a catalyst provides an alternative pathway for the reaction, which has a lower activation energy, allowing the reactants to go through the reaction more easily or quickly. The catalyst itself remains unchanged at the end of the reaction.

b) The addition of a catalyst decreases the activation energy of a reaction. Activation energy is the minimum energy required for a reaction to occur. By providing an alternate reaction pathway with a lower activation energy, a catalyst effectively lowers the energy barrier for the reaction, making it easier for the reactants to reach the transition state and proceed with the reaction.

c) The addition of a catalyst has no effect on the reaction enthalpy. Reaction enthalpy is a measure of the heat energy released or absorbed in a reaction, and it depends on the inherent properties of the reactants and products. A catalyst does not affect the thermodynamics of the reaction, only the kinetics.

d) The addition of a catalyst does not impact the equilibrium of a reaction. Catalysts increase both the forward and backward rates of a reaction, allowing the reaction to reach the equilibrium state more quickly. However, once the reaction reaches equilibrium, the relative concentrations of the reactants and products remain the same regardless of the presence of a catalyst. Therefore, the equilibrium position is unchanged by the addition of a catalyst.